Chemistry - Mole Concept Question with Solution | TestHub

ChemistryMole ConceptLaws of Chemical CalculationsMedium2 minQB

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Passage / Comprehension

A mixture of nitrogen and hydrogen. In the ratio of one mole of nitrogen to three moles of hydrogen, was partially converted into $NH_{3}$ so that the final product was a mixture of all these three gases. The mixture was to have a density of 0.5 g per litre at 0°C and 1.00 atm.

Calculate the % of $NH_{3}$ in the gaseous mixture, by volume. ( $22.4 \times 3.04 = 68$ )

Options:

Answer:

Solution:

Density = $0.5 g L^{- 1}$ at STP.

The molar mass of the mixture is $0.5 \times 22.4 = 11.2 g m o l^{- 1}$ .

Let $x$ moles of NH₃ be formed from the initial $1 m o l N_{2} + 3 m o l H_{2}$ .

The final moles are $(1 - x /2) + (3 - 3 x /2) + x = 4 - x$ . The total mass is $34 g$ .

The average molar mass is $\frac{34}{4 - x} = 11.2$ .

$4 - x \approx 3.04$

$x \approx 0.96$

The volume % of NH₃ is $\frac{0.96}{3.04} \times 100 = 31.6%$ .

Stream:JEESubject:ChemistryTopic:Mole ConceptSubtopic:Laws of Chemical Calculations

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